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Chemistry Module 15
Key Terms and Concepts from the Module
| Question | Answer |
|---|---|
| Chemical Equilibrium | The point at which both the forward and reverse reactions in a chemical equation have equal reaction rates: When this occurs, the amounts of each substance in the chemical reaction will not change, despite the fact that both reactions still proceed. |
| Equilibrium Constant | K = Products/Reactants with the Stochiometric Coefficients as superscripts |
| When K is large, the equilibrium is | weighted toward the products side of the equation |
| When K is small, the equilibrium is | weighted toward the reactants side of the equation |
| When K is near unity, the equilibrium is | balanced between reactants and products |
| When a solid appears in a chemical equilibrium | it is not included in Equation (15.2) |
| When a liquid appears in a chemical equation | we do not include it in Equation (15.2). This applies only to the liquid phase; it does not apply to the aqueous phase. |
| When a stress (such as a change in concentration, pressure, or temperature) is applied to an equilibrium | the reaction will shift in a way that relieves the stress and restores equilibrium |
| Le Chatelier's principle ignores solids and liquids | as a source of stress to the equilibrium |
| When an equilibrium is subjected to an increase in pressure | it will shift away from the side with the largest number of gas molecules |
| If pressure decreases | the equilibrium will shift toward the side with the largest number of gas molecules |
| If there are no gases in the equation or if the number of gas molecules are the same on both sides | nothing will happen |
| When temperature is raised, an equilibrium will shift | away from the side of the equation that contains energy |
| When temperature is lowered, the reaction will shift | toward the side that contains energy |
| acid ionization reactions | The reaction in which an H + separates from an acid molecule so that it can be donated in another reaction |
| acid ionization constant | The equilibrium constant for an acid's ionization reaction |
| If the ionization constant of an acid is large | the acid is considered a strong acid |
| If the ionization constant is not large | we call it a weak acid |
| In general, the larger the ionization constant | the stronger the acid |
| base ionization reaction | combined with water and accepts H+ |
| Solutions with pH 0 - 1.9 are considered | strongly acidic |
| solutions with pH 2 - 6.9 are considered | weakly acidic |
| solutions with pH 7.1 - 12 are considered | weakly basic |
| solutions with pH 12.1 - 14 are considered | strongly basic |
| A pH of 7 indicates a | neutral solution |
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